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Honors Chemistry NASD Int. High School Curriculum > 2014-2015 > Intermediate School > Science > Honors Chemistry

Thursday, February 5, 2015, 10:44AM

Last Updated: Monday, February 17, 2014 by Mark Anticole

Anticole, Mark; Gibson, Richelle; Jorden, Bill; Marnik, Jennifer; Uhernik, Leah; Zavacky, Brian Click on a Unit to edit your Curriculum

Essential Concepts

Key Learner Objectives (converted)

Resources / Content Assessment

The Use of Scientific Tools & Units of Measure (Week 1, 4 Weeks)

1. Laboratory work is an important and necessary component of chemistry. (7 days)

2. The Scientific Method is a scientific process used for problem solving. (3 days)

3. An accurate and consistent system of measurement is the foundation of modern chemistry. (10 days)

1. Laboratory work is an important and necessary component of chemistry. (7 days)

Investigate concepts by manipulating multiple variables, utilizing repeated trials and using basic error analysis.

Classify observations as qualitative and/or quantitative (CHEM.A.1.1.2)

Organize a set of data in a logical and coherent manner using appropriate tables, diagrams, charts, or graphs.

Write a conclusion for scientific investigation based on recorded qualitative and quantitative data that includes a statement of results, the relationship of the results to the hypothesis, an explanation and defense of the results, and an

Textbook

Introductory Chemistry: A Foundation, 5th Edition, Zumdahl; Chapters 1 and 2

Digital Media

Safety Videos

Graphing with Excel

Tutorials using Norton Website

CrashCourse Chemistry, "Unit Conversion & Significant

Figures" ( http://youtu.be/hQpQ0hxVNTg1)

CrashCourse Chemistry, "Lab Techniques & Safety" (http://youtu.be/VRWRmIEHr3A)

CrashCourse Chemistry, "The Global Carbon Cycle" (http://youtu.be/aLuSi_6Ol8M)

SciShow "The Times and Troubles of the Scientific Method" -

http://youtu.be/i8wi0QnYN6s

Tyler Dewitt Significant Figures Videos - http://www.youtube.com/playlist?list=PL3hPm0ZdYhyy0PQUQ1ka94hxVQPdYGS9m

Tyler Dewitt Scientific Notation Videos - http://www.youtube.com/playlist?list=PL3hPm0ZdYhyxZtI_OJ_tpyL_CPHq6_gvE

Tyler Dewitt Density Videos - http://www.youtube.com/playlist?list=PL3hPm0ZdYhyz_A3Q-jhLuGtBrWsJqTHpu

Additional Vocabulary

Erlenmeyer Flask

Graduated Cylinder

Equipment and Glassware Quiz

Measurement Quiz

Significant Figures Quiz

Unit 1 Exam Traditional Assessment: Written Test

Essential Concepts



analysis of possible sources of error.

Use mathematical manipulations in a laboratory setting (SI units, scientific notation, linear equations, graphing, ratio and proportion, dimensional analysis, use of scientific calculator).

Create an experimental design diagram that identifies the various levels of the independent variable, dependent variable, the control, the constants, and the number of trials.

Investigate and understand how to plan and conduct investigations in which instruments are selected and used to extend observations and measurements of mass, volume, temperature, heat exchange, etc.

Interpolate, extrapolate, and analyze trends to make predications and understand that the relationships between physical

Mortar and Pestle

Bunsen Burner

Pneumatic Trough

Gas Collecting Bottle

Buret

Pipet

Laboratory Exercises/Activities

Measurement of Matter Practice Packet

How to Light a Bunsen Burner

Introduction to Lab Techniques

Precision and Accuracy of Instruments

Density of Pennies

Metric Olympics

Density of Carbon Dioxide

Density Columns

Density of Ice, Water, and Alcohol

Density of Coke vs. Diet Coke

Equipment Use

Safety Equipment Use

Glass Bending

Safety Posters

Essential Concepts



quantities are determined using the shape of a curve passing through experimentally obtained data.

Use data to make inferences and predictions, or to draw conclusions, demonstrating understanding of experimental limits. (S11.A.2.1.3)

Communicate results of investigations using multiple representations. (S11.A.2.1.5)

Evaluate appropriate methods, instruments, and scale for precise quantitative and qualitative observations (e.g., to compare properties of materials, water quality). (S11.A.2.2.1)

Explain how technology is used to extend human abilities and precision (e.g., GPS, spectroscope, scanning electron microscope, pH meters, probes, interfaces, imaging

Essential Concepts



technologies, telescope). (S11.A.2.2.2)

Apply knowledge and understanding about the nature of scientific and technological knowledge. Know that science uses both direct and indirect observation means to study the world and the universe.

Describe materials using precise quantitative and qualitative skills based on observations.

Develop appropriate scientific experiments: raising questions, formulating hypotheses, testing, controlled experiments, recognizing variables, manipulating variables, interpreting data, and producing solutions.

Demonstrate designated laboratory techniques and safe usage of chemicals and equipment, in addition to proper

Essential Concepts



response to emergency situations.

Use appropriate technology for gathering and analyzing data and communicating results (i.e. probeware, Microsoft Office Programs).

Follow precisely a complex multi step procedure when carrying out experiments, taking measurements, or performing technical tasks, attending to special cases or exceptions defined in the text. (CC.3.5.9-10.C)

Write routinely over extended time frames (time for reflection and revision) and shorter time frames (a single sitting or a day or two) for a range of discipline-specific tasks, purposes, and audiences. (CC.3.6.9-10.I)

2. The Scientific Method is a scientific process used for problem solving. (3 days)

Participate both as an individual and as a team member on

Essential Concepts



scientific investigations.

Understand that hypotheses are formulated based on prior knowledge and observations.

Recognize and discuss the limitations of the experimental apparatus and design.

Translate a description of a physical problem into a mathematical statement in order to find a solution.

Evaluate the appropriateness of research questions (e.g., testable vs. not-testable). (S11.A.1.1.3)

Use appropriate quantitative data to describe or interpret change in systems (e.g., biological indices, electrical circuit data, automobile diagnostic systems data). (S11.A.1.3.1)

Critique the elements of an experimental design (e.g., raising questions, formulating hypotheses, developing

Essential Concepts



procedures, identifying variables, manipulating variables, interpreting data, and drawing conclusions) applicable to a specific experimental design. (S11.A.2.1.1)

Critique the elements of the design process (e.g. identify the problem, understand criteria, create solutions, select solution, test/evaluate and communicate results) applicable to a specific technological design. (S11.A.2.1.2)

Use appropriate quantitative data to describe or interpret a system (e.g., biological indices, electrical circuit data, automobile diagnostic systems data). (S11.A.3.1.3)

Describe concepts of models as a way to predict and understand science and technology.

Cite specific textual evidence to support analysis of science

Essential Concepts



and technical texts, attending to the precise details of explanations or descriptions. (CC.3.5.9-10.A)

Write arguments focused on disciplined specific content. (CC.3.6.9-10.A)

Produce clear and coherent writing in which the development, organization, and style are appropriate to task, purpose, and audience. (CC.3.6.9-10.C)

Use technology, including the Internet, to produce, publish, and update individual or shared writing products, taking advantage of technology's capacity to link to other information and to display information flexibly and dynamically. (CC.3.6.9-10.E)

3. An accurate and consistent system of measurement is the foundation of modern chemistry. (10 days)

Utilize metric units in all measurements and calculations.

Recognize the

Essential Concepts



limitations of measured quantities through appropriate use of significant figures or error ranges.

Use appropriate conversions to incorporate data gathered from non-SI instruments.

Apply mathematical models to science and technology.

Apply scale as a way of relating concepts and ideas to one another by some measure.

Apply dimensional analysis and scale as a ratio.

Apply scale as a way of relating concepts and ideas to one another by some measure. Convert one scale to another.

Describe patterns of change in nature, physical and man-made systems. Describe the effects of error in measurements.

Write numeric quantities in standard and scientific notation.

Add, subtract, multiply, and divide numbers written in

Essential Concepts



scientific notation.

Identify the fundamental quantities of the metric system.

Perform dimensional analysis in calculations.

Convert quantities between and among the metric and English systems of measurement.

Vocabulary of Chemistry (Week 5, 2 Weeks)

1. Chemistry is the study of matter, and to be science literate, there are multiple terms and expressions that must be used to describe matter. (2 days)

2. Matter can be described by its properties and classified into multiple categories. (4 days)

3. Mixtures can be separated

1. Chemistry is the study of matter, and to be science literate, there are multiple terms and expressions that must be used to describe matter. (2 days)

Apply system analysis, showing relationships (e.g. flowcharts, decision trees, dichotomous keys, mind map), input and output, and measurements to explain a system and its parts. (S11.A.3.1.1)

Analyze the structure of the relationships among concepts in a text, including relationships among key terms. (e.g., energy). (CC.3.5.9-10.E)

2. Matter can be described by its properties and

Textbook

Introductory Chemistry: A Foundation, 5th Edition, Zumdahl; Chapters 1 and 2

Digital Media

Four Weddings and a Friendship Video

Physical Chemical Changes Video

Elements Video

Additional Vocabulary Laboratory Exercises/Activities

Changes in Matter

Baggie Lab

Conservation of Matter

Solid X/Liquid Y

Summary Lab of Vocabulary

Density of Pennies

Separation of a Mixture

Physical/Chemical Changes

Tyndall Effect

Physical and Chemical Properties/Change Quiz

Element Names and Symbols Written Test


Essential Concepts



by physical means. (4 days)

classified into multiple categories (4 days)

Describe how relationships represented in models are used to explain scientific or technological concepts (e.g., difference between elements, compounds, and mixtures at the particle level.) (S.11.A.3.2.3)

Differentiate between homogeneous and heterogeneous mixtures (CHEM.A.1.2.2)

Apply process knowledge and organize scientific and technological phenomena in varied ways.

Describe materials using precise quantitative and qualitative skills based on observations.

Distinguish between physical and chemical properties and also between simple physical and chemical changes.

Differentiate between the three states of matter.

Compare stationary physical patterns (e.g., molecular structure and arrangement) to the object’s properties. (S11.A.3.3.2)

Predict how combinations of substances can results in physical and/or chemical changes.

Classify matter as elements, compounds, or mixtures.

Apply the law of definite proportions to the

Essential Concepts



classification of elements and compounds as pure substances. (CHEM.B.1.2.2)

1. Mixtures can be separated by physical means. (4 days)

Participate both as an individual and as a team member on scientific investigations.

Investigate and understand how to demonstrate scientific reasoning and logic.

Explain how specific scientific knowledge or technological design concepts solve practical problems (e.g., separation of mixtures). (S11.A.1.1.4)

Evaluate appropriate methods, instruments, and scale for precise quantitative and qualitative observations (e.g., to compare properties of materials, water quality). (S11.A.2.2.1)

Analyze and predict the effect of making a change in one part

Essential Concepts



of a system on the system as a whole. (S11.A.3.1.2)

Compare the accuracy of predictions represented in a model to actual observations and behavior.

Apply process knowledge and organize scientific and technological phenomena in varied ways. Develop appropriate scientific experiments: raising questions, formulating hypotheses, testing, controlled experiments, recognizing variables, manipulating variables, interpreting data, and producing solutions.

Apply the elements of scientific inquiry to solve problems. Generate questions about objects, organisms and/or events that can be answered through scientific investigations.

Apply the elements of scientific inquiry

Essential Concepts



to solve problems. Conduct a multiple step experiment.

Apply the elements of scientific inquiry to solve problems. Organize experimental information using a variety of analytical methods.

Apply the elements of scientific inquiry to solve problems. Judge the significance of experimental information in answering the question.

Apply the elements of scientific inquiry to solve problems. Suggest additional steps that might be done experimentally.

Identify and apply the technological design process to solve problems. Propose and analyze a solution.

Identify and apply the technological design process to solve problems. Implement the solution.

Identify and apply the technological design process to solve problems.

Essential Concepts



Evaluate the solution, test, redesign and improve as necessary.

Demonstrate designated laboratory techniques and safe usage of chemicals and equipment, in addition to proper response to emergency situations.

Use appropriate technology for gathering and analyzing data and communicating results (i.e. probeware, Microsoft Office Programs).

Identify and safely use a variety of tools, basic machines, materials and techniques to solve problems and answer questions. Select and safely apply appropriate tools, materials and processes necessary to solve complex problems.

Thermochemistry (Week 7, 3 Weeks)

1. All physical and chemical changes are

1. All physical and chemical changes are accompanied by changes in energy. (6 days)

Textbook

Introductory Chemistry: A Foundation, 5th Edition, Zumdahl;

Unit 3 Exam Traditional Assessment:

Essential Concepts



accompanied by changes in energy. (6 days)

2. The kinetic theory of heat and temperature explains the flow of energy in systems. (5 days)

3. Changes in Energy can be quantitatively measured using a calorimeter. (4 days)

Identify exothermic and endothermic reactions.

Give examples of different forms of energy.

Describe energy changes in chemical reactions. (S11.C.2.1.2)

Analyze energy sources and transfers of heat. Evaluate energy changes in chemical reactions. (3.4.10.B.3)

Define enthalpy, and relate enthalpy change in a process occurring at constant pressure to the heat added to or lost by the system during the process.

Sketch an energy diagram, given the enthalpy changes in the process involved, and associate the sign of delta H with whether the process is endothermic or exothermic.

Calculate the quantity of heat involved in a reaction at constant pressure given the quantity or reactants and the enthalpy change for the

Chapters 1 and 2

Digital Media

Graphing with Heating/Cooling Curve

Derivation of the Three Temperature Scales

"The Race for Absolute Zero" Video

CrashCourse Chemistry, "Energy & Chemistry" (http://youtu.be/GqtUWyDR1fg)

CrashCourse Chemistry, "Enthalpy" (http://youtu.be/SV7U4yAXL5I)

CrashCourse Chemistry, "Calorimetry" (http://youtu.be/JuWtBR-rDQk)

CrashCourse Chemistry, "Entropy" (http://youtu.be/ZsY4WcQOrfk)


Calorimetry

Bomb Calorimeter

Coffee Cup Calorimeter

Hot Water Bath


Specific Heat of a Metal

Temperature of a Bunsen Burner

Heating/Cooling Curve of a Pure Substance

Food Calorimetry

Barium Hydroxide/Ammonium Thiocyanate

Sulfuric Acid and Sugar

Sugar and Potassium Chlorate

Jolly Rancher/Water and Jolly Rancher/Potassium Chlorate

Written Test

Essential Concepts



reaction on a mole basis.

Describe patterns of change in nature, physical and man-made systems. Describe changes to matter caused by heat, cold, light or chemicals using a rate function. (3.1.10.E.4)

2. The kinetic theory of heat and temperature explains the flow of energy in systems. (5 days)

Apply the knowledge of conservation of energy to explain common systems (e.g., refrigeration system, rocket propulsion, heat pump). (S11.C.2.1.3)

Analyze energy sources and transfers of heat. Use knowledge of conservation of energy and momentum to explain common phenomena (e.g., refrigeration system, rocket propulsion). (3.4.10.B.4)

Describe factors that influence the frequency of collisions during chemical reactions

Essential Concepts



that might affect the reaction rates (e.g., surface area, concentration, catalyst, temperature, agitation). (S11.C.1.1.6)

Recognize and analyze alternative explanations and models.

Compare and contrast scientific theories, scientific laws, and beliefs (e.g., the law of gravity, how light travels, formation of moons, stages of ecological succession). (S11.A.1.1.1)

Investigate and understand how evaluation of evidence for scientific theories and how new discoveries, may either modify existing theories or result in establishing a new paradigm.

Evaluate appropriate methods, instruments, and scale for precise quantitative and qualitative observations (e.g., to compare

Essential Concepts



properties of materials, water quality). (S11.A.2.2.1)

Use appropriate quantitative data to describe or interpret a system (e.g., biological indices, electrical circuit data, automobile diagnostic systems data). (S11.A.3.1.3)

Apply scale as a way of relating concepts and ideas to one another by some measure. Convert one scale to another. (3.1.10.D.2)

3. Changes in Energy can be quantitatively measured using a calorimeter. (4 days)

Define the terms heat capacity and specific heat.

Calculate any one of the following quantities given the other three: heat, quantity of material, temperature change, and specific heat.

Calculate the heat absorbed or evolved when a given quantity of a substance changes from one condition to another using

Essential Concepts



heat capacities and enthalpies for phase changes.

Use appropriate conversions to incorporate data gathered from non-SI instruments.

Utilize metric units in all measurements and calculations

Recognize the limitations of measured quantities through appropriate use of significant figures or error ranges.

Organize a set of data in a logical and coherent manner using appropriate tables, diagrams, charts, or graphs.

Apply process knowledge and organize scientific and technological phenomena in varied ways. Develop appropriate scientific experiments: raising questions, formulating hypotheses, testing, controlled experiments, recognizing variables, manipulating variables, interpreting data,

Essential Concepts



and producing solutions. (3.2.10.B.2)

Translate quantitative or technical information expressed in words in a text into visual form (e.g., a table or chart) and translate information expressed visually or mathematically (e.g., in an equation) into words. (CC.3.5.9-10.G)

Atomic and Quantum Theories (Week 10, 4 Weeks)

1. The atomic model has evolved based on the ideas and experiments of many accomplished scientists. (1 week)

2. Scientists can use indirect observation to analyze patterns and to draw conclusions. (1 week)

3. The electron has both wave and particle properties.

1. The atomic model has evolved based on the ideas and experiments of many accomplished scientists. (1 week)

Recognize the contributions made by scientists throughout culture, and explain how scientific knowledge builds and changes over time.

Trace the idea of the atom from early Greek civilization to the modern era.

Compare and contrast scientific theories, scientific laws, and (S11.A.1.1.1)

Describe how

Textbook

Introductory Chemistry, A Foundation; 5th Edition, Zumdahl; Chapters 4 and 10

Digital Media

Three 10-minute History Videos

Historical Experiments Videos

TED-ED, "Just How Small is an Atom?" (http://ed.ted.com/lessons/just-how-small-is-an-atom)

CrashCourse Chemistry, "The Nucleus" (http://youtu.be/FSyAehMdpyI)

CrashCourse Chemistry, "The Electron" (http://youtu.be/rcKilE9CdaA)

CrashCourse Chemistry, "The History of Atomic Chemistry" (

http://youtu.be/thnDxFdkzZs)

CrashCourse Chemistry, "Nuclear Chemistry" (http://youtu.be/KWAsz59F8gA)

CrashCourse Chemistry, "Fusion & Fission" (http://youtu.be/FU6y1XIADdg)

Parts of the Atom Quiz

Electron Configurations Quiz


Essential Concepts



(1 week) 4. The

quantum model of the atom contains a nucleus and electron clouds that are described by four quantum numbers and electron configurations. (1 week)

relationships represented in models are used to explain scientific or technological concepts. (S11.A.3.2.3)

Relate the physical properties of matter to its atomic or molecular structure (CHEM. A.1.1.4)

Describe the composition of an atom in terms of protons, neutrons, and electrons.

Give the approximate size, relative mass, and charge of an atom, proton, neutron, and electron.

Write the chemical symbol for an element, having been given its mass number and atomic number, and perform the reverse operation.

Differentiate between the mass number of an isotope and the average atomic mass of an element. (CHEM. A.2.1.2)

Write the symbol and charge for an atom or ion, having been given the


Spectroscopic Notation

Radioactivity

Types of Electromagnetic Radiation

Relativity

Lewis Dot Structures


Gold Penny

Flame Test

Fireworks

Mystery Atomic Box

Isotopes of Pennies

Candium Lab

Beanium Lab

Basketball and Frequency

Spectral Tubes

Standing Waves

Combustion of Alcohol and Salt

Radioactive Isotope Activity using Skittles

Wanted Element Posters

rutherfore exp demo

orbital hybridization demo

orbital pictures and drawing program

http://micro.magnet.fsu.edu/electromag/java/rutherford/http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/hybrv18.swfhttp://www.orbitals.com/orb/http://micro.magnet.fsu.edu/electromag/java/rutherford/http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/hybrv18.swfhttp://www.orbitals.com/orb/

Essential Concepts



number of protons, neutrons, and electrons, and perform the reverse operation.

Calculate the atomic mass/weight of an element given the abundances and masses of its isotopes.

Use the periodic table to predict the charges of monatomic ions.

Explain that matter is made of particles called atoms and that atoms are composed of even smaller particles (e.g., proton, neutrons, electrons). (S11.C.1.1.1)

Scientists can use indirect observation to analyze patterns and to draw conclusions. (1 week)

Describe the evolution of atomic theory leading to the current model of the atom based on the works of Dalton, Thomson, Rutherford and Bohr. (CHEM A.2.1.1)

Understand that

Essential Concepts



hypotheses are formulated based on observations.

Investigate and understand how to demonstrate scientific reasoning and logic.

Investigate and understand how evaluation of evidence for scientific theories and how new discoveries, may either modify existing theories or result in establishing a new paradigm.

Analyze and explain how to verify the accuracy of scientific facts, principles, theories, and laws. (S11.A.1.1.2)

Compare and contrast findings presented in a text to those from other sources (including their own experiments), noting when the findings support or contradict previous explanations or accounts. (CC.3.5.9.10I)

2. The electron has both wave and particle properties. (1 week)

Describe the

Essential Concepts



properties of an electron as seen in cathode rays.

Cite the evidence from studies of radioactivity for the existence of subatomic particles.

Relate quantitatively wavelength, frequency, and energy for electromagnetic radiation.

Explain the nature of Planck's quantum theory.

Explain what is meant by bright line or line emission spectra.

List the assumptions made by Bohr in his model of the hydrogen atom.

Relate the existence of quantized energy levels to atomic emission spectra. (CHEM. A.2.2.4)

Explain the concept wave/particle duality.

3. The quantum model of the atom contains a nucleus and electron clouds that are described by four quantum numbers and electron configurations. (1 week)

Predict the ground state electronic

Essential Concepts



configuration and/or orbital diagram for a given atom or ion. (CHEM. A.2.2.1)

Describe Heisenberg's uncertainty principle and explain the limitation it places on our ability to define simultaneously the location and momentum of a subatomic particle, particularly the electron.

Explain the concepts of orbital, electron density, and probability as used in the quantum mechanical model of the atom.

Identify the types and shapes of subshells in an energy shell of an atom.

Explain why electrons with the same principal energy level but different sublevels possess different energies.

Explain the concept of electron spin.

State Hund's Rule and illustrate how it is used in writing the

Essential Concepts



electronic structures of the elements.

Write the electron configurations for any element using the placement of the element in the periodic table.

Describe what is meant by the s, p, d, and f blocks.

History of the Periodic Table and Periodicity (Week 14, 2 Weeks)

1. The work of many scientists has led to the development of the Modern Periodic Table. (1 days)

2. Repeatable patterns can be observed on the Periodic Table which lead to the ability to make predictions and intelligent guesses about the unknown properties of elements and their

1. The work of many scientists has led to the development of the Modern Periodic Table. (1 day)

Compare early and modern periodic tables.

2. Repeatable patterns can be observed on the Periodic Table which lead to the ability to make predictions and intelligent guesses about the unknown properties of elements and their compounds. (7 days)

Use the periodic table to predict whether an element is a metal, metalloid, or nonmetal.

Cite and explain the general trends and deviations in ionization energy, atomic radii, electronegativit

Textbook

Introductory Chemistry: A Foundation, 5th Edition, Zumdahl; Chapter 10 and 11

Digital Media

Reactivity of Alkali Metals and Water Video Clips

Graphing the Trends of the Periodic Table

CrashCourse Chemistry - "The Creation of Chemistry - "The

Fundemental Laws" ( http://youtu.be/QiiyvzZBKT8)

CrashCourse Chemistry - "The Periodic Table" (http://youtu.be/0RRVV4Diomg)

Tyler Dewitt Atomic Radius and Ionization Energy Video - http://www.youtube.com/watch?v=Mmti4kKDcqA

SciShow Video on Dmitri Mendeleev - http://www.youtube.com/watch?v=IgA37CNa7Ow&list=PLC31B0C382F9585D6&index=4


Periodicity

Effective Nuclear Charge (ENC)

Shielding Effect


Periodic Trends Quiz


Essential Concepts



compounds. (7 days)

3. Elements that are in the same group have similar outer electronic configurations and often behave in a similar manner to one another. (2 days)

y and electron affinity that occur in specific groups and series within the periodic table. (CHEM.A.2.3.2)

Describe how the radii of ions relate to those parent atoms.

Explain the concept of an isoelectronic series and the origin of changes in ionic radius within such a series.

Describe the periodic trends in metallic and nonmetallic behavior.

Describe the general differences in chemical reactivity between metals and nonmetals.

Describe general physical and chemical behavior of the alkali metals and alkaline earth metals, and explain how their chemistry relates to their position on the periodic table.

Explain the very low chemical reactivity of the noble gas elements.

Explain how the relationships of

Investigation of Alkali Metals and Alkaline Earth Metals

Investigation of Halogens

Investigation of Metals/Nonmetals/Metalloids

Reactivity Series

Alkali Metal Reactivity

Atomic/Ionic Size Trend

Electron Affinity Trend

Prediction of Properties of Unknown Elements

Five Atom Mystery

Alien Periodic Table

Essential Concepts



chemical properties of elements are represented in the repeating patterns within the periodic table. (S11.C.1.1.4)

Explain how the periodicity of chemical properties lead to the arrangements of elements on the periodic table. (CHEM.A.2.3.1)

Recognize when the octet rule applies to the arrangement of electrons in the valence shell for any atom

Gather relevant information from multiple authoritative print and digital sources, using advanced effectively; assess the usefulness of each source in answering the research question; integrate information into the text selectively to maintain the flow of ideas, avoiding plagiarism and following a standard format for citation. (CC.3.6.9-10.G)

3. Elements that are in the

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same group have similar outer electronic configurations and often behave in a similar manner to one another. (2 days)

Explain the relationship between the physical properties of a substance and its molecular or atomic structure. (S11.C.1.1.2)

Explain the repeating pattern of chemical properties by using the repeating patterns of atomic structure within the periodic table. (3.4.10.A.2)

Chemical Formulas and Nomenclature (Week 16, 4 Weeks)

1. The are three main types of chemical formulas (empirical, molecular, and structural) that are used to describe the composition of a compound. (2 days)

2. Atoms combine to form

1. The are three main types of chemical formulas (empirical, molecular, and structural) that are used to describe the composition of a compound. (2 days)

Define empirical, molecular and structural formulas.

Distinguish among the three types of formulas.

Write the symbol and charge for an atom or ion, having been given the number of protons, neutrons, and

Textbook

Introductory Chemistry, A Foundation; 5th Edition; Zumdahl; Chapter 5

Digital Media

Norton Tutorials

CrashCourse Chemistry, "Nomenclature" (http://youtu.be/mlRhLicNo8Q)


Hydrocarbon

Expanded and Condensed Structural Formulas


Predicting Stable Ion Charges Quiz

Naming Compounds Quiz


Essential Concepts



compounds by changing their electron configurations in order to become more stable. (1 day)

3. Formulas for ionic and covalent compounds are written in two different ways. (8 days)

4. There are three systems (stock, classical, and informal/common) of naming compounds so it is important to understand and use all three systems. (8 days)

electrons, and perform the reverse operation.

Write the simplest formula for an ionic or covalent compound.

Predict on the basis of the periodic table the probable formulas of ionic substances formed between common metals and nonmetals.

2. Atoms combine to form compounds by changing their electron configurations in order to become more stable. (1 day)

Write the electron configurations representing atomic stability.

3. Formulas for ionic and covalent compounds are written in two different ways. (8 days)

Define ionic and covalent compounds.

Utilize simple rules and the location of the element on the periodic table to predict compound type.

Utilize the “criss-cross” method to write formulas for binary and ternary ionic compounds.

Copper Cycle Lab

What's Your Name Activity

Chromatography of Metallic Ions

Essential Concepts



Apply the rules for naming and writing formulas for binary molecular compounds.

4. There are three systems (stock, classical, and informal/common) of naming compounds so it is important to understand and use all three systems. (8 days)

Apply a systematic set of rules (IUPAC) for naming compounds and writing chemical formulas (e.g. binary covalent, binary ionic, ionic compounds containing polyatomic ions). (CHEM.A.1.1.5)

Apply the rules for naming binary and oxyacids.

Write the name of an ionic and/or covalent compound using both the classical and stock systems.

Chemical Reactions (Week 20, 3 Weeks)

1. A chemical reaction is the process by which one or more substances change into one or more

1. A chemical reaction is the process by which one or more substances change into one or more different substances. (2 days)

Describe how to write a word equation.

Textbook

Introductory Chemistry, A Foundation; 5th Edition; Zumdahl; Chemical Reactions; Chapters 6 and 7

Digital Media

Balancing Equations Quiz

Predicting Products Quiz

Essential Concepts



different substances. (2 days)

2. There are hundreds of different kinds of chemical reactions, but many can be divided into 5 general categories. (7 days)

3. Once a chemist knows the type of reaction, they can then predict the products of the reaction. (3 days)

4. Chemical equations can be written in three forms: molecular, complete ionic, and net ionic. (3 days)

Describe how to write a skeleton equation.

Describe the steps for writing a complete chemical equation.

Describe factors that influence the frequency of collisions during chemical reactions that might affect the reaction rates (e.g. surface area, concentration, catalyst, temperature). (S.11.C.1.1.6)

2. There are hundreds of different kinds of chemical reactions, but many can be divided into 5 general categories. (7 days)

Balance chemical equations by applying the Law of Conservation of Matter. (CHEM.B.2.1.5)

Describe and identify the five general types of chemical reactions.

Classify reactions as synthesis, decomposition, single replacement, double replacement, or combustion. (CHEM.B.2.1.3)

3. Once a chemist knows the type of reaction, they can

Chem Balancer Tutorial

Virtual Determination of an Activity Series

TED-ED, "How To Speed Up a Chemical Reaction" (http://ed.ted.com/lessons/how-to-speed-up-chemical-reactions-and-get-a-date)

CrashCourse Chemistry, "Precipitation Reactions" (http://youtu.be/IIu16dy3ThI)

CrashCourse Chemistry, "Redox Reactions" (http://youtu.be/lQ6FBA1HM3s)

CrashCourse Chemistry, "Types of Reactions" (http://youtu.be/QXT4OVM4vXI)


Oxidation

Reduction

Redox Reactions

Laboratory Exercises/Activites

Precipitation Lab

Types of Reactions Lab

The Copper Cycle

Miscellaneous Reactions

Redox Titration

Tin Sponge

Elephant Toothpaste

Genie in Bottle

Thermite Reaction

Sweet 16 Prediction of a Product

Switching Partner Activity

Net Ionic Equations Quiz


Essential Concepts



then predict the products of the reaction. (3 Days)

Predict the products of the five general types of chemical reactions. (CHEM.B.2.1.4)

Define precipitate and determine the solubility of products in a double replacement reaction.

Interpret the, “Solubility Chart,” to predict products of a double replacement reaction.

Interpret the, “Activity Series of the metals,” to predict products of a single replacement reaction.

Distinguish between complete and incomplete combustion reactions.

Predict the products of complete and incomplete combustion reactions.

4. Chemical equations can be written in three forms: molecular, complete ionic, and net ionic. (3 days)

Write a complete ionic equation.

Determine the spectator ions.

Determine the

Essential Concepts



precipitate or molecular compound product.

Write the net ionic equation.

The Mole Concept and Stoichiometry (Week 23, 3 Weeks)

1. Chemists are interested in the quantity of an element or compound (number of atoms, molecules, or formula units); however, these entities are much too small to count individually, so chemists use a unit called the mole to count by massing them. (2 days)

2. One mole always contains the same number of particles (Avogadro's number), no matter what

1. Chemists are interested in the quantity of an element or compound (number of atoms, molecules, or formula units); however, these entities are much too small to count individually, so chemists use a unit called the mole to count by massing them (2 Days)

Describe methods of measuring the amount of a sample.

Define representative particle.

Identify and distinguish between the different types of representative particles: atom, molecule, formula unit, and ion.

Distinguish between atomic mass of an element and its molar mass.

2. One mole always contains the same number of particles (Avogadro's number), no matter what the substance. (2 days)

Define Avogadro’s number as it related to a mole of a substance.

Textbook

Introductory Chemistry, A Foundation; 5th Edition; Zumdahl; Chapter 8 and 9

Digital Media

TED-ED, "How Big is a Mole?" (http://ed.ted.com/lessons/daniel-dulek-how-big-is-a-mole-not-the-animal-the-other-one)

CrashCourse Chemistry - "Stoichiometry" (http://youtu.be/UL1jmJaUkaQ)


Empirical Formula of Magnesium Oxide

Identification of Metals through Molar Mass

Determination of the Empirical Formula of a Hydrate

Using Stoichiometry to Determine the Mass of Carbon Dioxide Production

Using Stoichiometry to determine the Percent Yield of Silver

Mole to Dozen Analogy

Avogadro's Number of Real World Substances

The Chalk Mole Lab

Percent Composition of Gum

Percent Composition of an Oreo

Making Smores

Basics of Stoichiometry Quiz


Essential Concepts



the substance. (2 days)

3. Stoichiometry is the part of chemistry that deals with the amounts of substances involved in chemical reactions. (6 days)

4. By writing balanced chemical equations and incorporating mole conversions, chemists can calculate the amount of reactants needed or the amount of products produced. (5 days)

Describe how the mass of one mole of a compound is calculated.

Apply the mole concept to representative particles (e.g counting, determining mass of atoms, ions, molecules, and/or formula units). (CHEM.B.1.1.1)

3. Stoichiometry is the part of chemistry that deals with the amounts of substances involved in chemical reactions. (6 days)

Describe how to convert the mass of a substance to the number of moles of a substance and visa versa.

Utilize dimensional analysis to solve problems involving moles, molecules, grams, ions, and atoms.

Calculate the percent by mass of an element in a compound.

Relate the percent composition and mass of each element present in a compound. (CHEM.B.1.2.3)

Determine the

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empirical and molecular formulas of compounds. (CHEM.B.1.2.1)

4. By writing balanced chemical equations and incorporating mole conversions, chemists can calculate the amount of reactants needed or the amount of products produced. (5 days)

Interpret balanced chemical equations in terms of moles, representative particles, and mass.

Use stoichiometric relationships to calculate the amounts of reactants and products involved in a chemical reaction. (CHEM.B.2.1.2)

Apply the mole concept, or Avogadro’s number, in stoichiometric calculations, including those involving limiting reactants and percent yield.

Identify and use the limiting reagent in a reaction to calculate the maximum amount of product(s) produced and the amount of excess reagent that

Essential Concepts



remains unreacted.

Calculate theoretical yield, actual yield, or percent yield given appropriate information.

Describe the roles of limiting and excess reactants in chemical reactions. (CHEM.B.2.1.1)

Use data to make inferences and predictions, or to draw conclusions, demonstrating understanding of experimental limits. (S.11.A.2.1.3)

Predict the amounts of reactant and products involved in a chemical reaction using molar volume of a gas at STP. (CHEM.B.2.2.2)

Chemical Bonding (Week 26, 3 Weeks)

1. Bonding is the linkage of atoms that form compounds through the transfer or sharing of valence electrons. (2 weeks)

2. Bonding has a profound effect on chemical

1. Bonding is the linkage of atoms that form compounds through the transfer or sharing of valence electrons. (2 weeks)

Recognize and describe different types of models that can be used to illustrate the bonds that hold atoms together in a compound (e.g. ball-and-stick

Textbook Introductory Chemistry, A Foundation; 5th Edition; Zumdahl; Chapter 11 Digital Media Norton Tutorial - Why Atoms Bond?

Tyler Dewitt Ionic vs. Molecular Compounds Video - http://www.youtube.com/watch?v=yADrWdNTWEc

Writing Ionic Formulas Video - http://www.youtube.com/watch?v=URc75hoKGLY

Writing Formulas with Polyatomic Ions - http://www.youtube.com/watch?v=p9iQ5Qn42DM

Ionic Bonding Introduction Video - http://www.youtube.com/watch?v=Qf07-8Jhhpc Additional Vocabulary

Identify the Different Types of Bonds and Their Properties Quiz

Lewis Structures Quiz

Unit Exam Written Test

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and physical properties. (1 week)

models, skeletal formulas, Lewis dot structures). (CHEM.B.1.4.1)

Chemical bonding can be described as covalent, polar covalent, ionic, or metallic. (8 days)

Classify a bond as being polar covalent, non-polar covalent, or ionic. (CHEM.B.1.3.2)

Use illustrations to predict the polarity of a molecule. (CHEM.B.1.3.3)

Explain how atoms combine to form compounds through ionic and covalent bonding. (CHEM.B.1.3.1)

Describe the arrangement of atoms in a metal.

Utilize Lewis dot structures to predict the structure and bonding in simple compounds. (CHEM.B.1.4.2)

Understand that resonance structures must be used to demonstrate when it is possible to draw two or more valid Lewis structures.

Describe how electrons are shared


Properties of Covalent and Ionic Bonding

Alum Crystals

Conductivity of Solutions

Crystal Lattice with Gum Drops

Essential Concepts



to form covalent bonds and identify exceptions to the octet rule.

Describe how atoms form double and triple covalent bonds.

Describe how electronegativity values determine the distribution of charge in a polar molecule.

2. Bonding has a profound effect on chemical and physical properties. (1 week)

Use bonding types to determine a substance’s physical properties such as melting point, boiling point, electrical conductivity, water solubility, and vapor pressure.

Explain the nature and importance of alloys.

Explain the formation of compounds (ionic and covalent) and their resulting properties using bonding theories. (S.11.C.1.1.3)

Distinguish between melting and boiling points of molecular compounds and

Essential Concepts



ionic compounds.

Describe how chemical bonding can affect whether a substance dissolves in a given liquid. (CHEM.A.1.2.5)

VSEPR Theory and Intermolecular Forces (Week 29, 2 Weeks)

1. The macroscopic properties of matter are a consequence of its molecular structure. (1 day)

2. The arrangement of electrons around the atoms predicts the shapes of molecules and ions. (1 week)

3. Three types of intermolecular forces exist between neutral molecules or atoms: dipole-dipole forces, London forces, and

1. The macroscopic properties of matter are a consequence of its molecular structure. (1 day)

Relate physical properties (boiling point, melting point, isomers, etc.) to molecular properties.

2. The arrangement of electrons around the atoms predicts the shapes of molecules and ions. (1 week)

Describe how VSEPR theory helps predict the shapes of molecules.

Describe the polarity of a molecule.

Use illustrations to predict the polarity of a molecule. (CHEM.B.1.3.3)

Utilize Lewis dot structures to predict the structure and bonding in simple compounds. (CHEM.B.1.4.2)

Textbook Introductory Chemistry, A Foundation; 5th Edition; Zumdahl; Chapter 11 Digital Media

Video clips/simulations showing attractive and repulsion forces

Senior Chemistry Video - Electron Arrangements and Bonding

Tyler Dewitt VSEPR Videos - http://www.youtube.com/playlist?list=PL3hPm0ZdYhyw5Gn0nUgH7809B6W7sLP3s

CrashCourse Chemistry, "Polar & Non-Polar Molecules" (http://youtu.be/PVL24HAesnc)

CrashCourse Chemistry, "Bonding Models and Lewis

Structures" ( http://youtu.be/a8LF7JEb0IA)

CrashCourse Chemistry, "Orbitals" (http://youtu.be/cPDptc0wUYI)


Freezing of Water

Bending of Water

VSEPR with Candy

VSEPR with Balloons

Bonds and IAF's

VSEPR Quiz

IMF Quiz


http://www.bcpl.net/~kdrews/interactions/interactions.htmlhttp://www.bcpl.net/~kdrews/interactions/interactions.html

Essential Concepts



hydrogen bonding forces. (4 days)

3. Three types of intermolecular forces exist between neutral molecules or atoms: dipole-dipole forces, London forces, and hydrogen bonding forces. (4 days)

Define Van der Waal's forces, dipole moment, hydrogen bonding, and electrostatic attraction.

Compare the strength of the intermolecular forces.

Evaluate the strength of intermolecular attractions as compared to the strength of ionic and covalent bonds.

Determine the type of intermolecular forces found between molecules.

Behavior of Gases (Week 31, 2 Weeks)

1. The ideal gas law is given by the equation: PV=nRT. (2 days)

2. All gases behave quite simply with respect to temperature, pressure,

1. The ideal gas law is given by the equation: PV=nRT. (2 days)

Define direct and inverse relationships.

Define an ideal gas.

Use the Ideal Gas Law to determine the relationship between the variables.

Textbook


Digital Media

Video Simulation showing relationships of pressure, volume, and temperature

TED-ED, "The ABC's of Gases" (http://ed.ted.com/lessons/1207-1-a-bennet-brianh264)

ASSESSMENT OVERRIDE


Essential Concepts



volume, and molar amount. By holding two of these physical properties constant, it becomes possible to show a simple relationship between the other two properties. (7 days)

3. The reference condition for gases, chosen by convention, is exactly 0°C and 1 atm pressure. (1 day)

Use the Ideal Gas Law to calculate the pressure, volume, temperature or moles of a gas.

2. All gases behave quite simply with respect to temperature, pressure, volume, and molar amount. By holding two of these physical properties constant, it becomes possible to show a simple relationship between the other two properties. (7 days)

Explain, using Kinetic Molecular Theory, why gases are easier to compress than solids or liquids.

Define pressure and identify units of pressure.

Utilize dimensional analysis to convert between units of pressure.

Relate the mass, velocity, and kinetic energy of a moving gas molecule.

Utilize mathematical relationships to predict changes in the number of particles, the temperature, the pressure, and the volume in a gaseous system (i.e. Boyle’s

CrashCourse Chemistry, "The Ideal Gas Law" (http://youtu.be/BxUS1K7xu30)

CrashCourse Chemistry, "Ideal Gas Law Problems" (http://youtu.be/8SRAkXMu3d0)

CrashCourse Chemistry, "Real Gases" (http://youtu.be/GIPrsWuSkQc)

CrashCourse Chemistry, "Partial Pressures & Vapor Pressure"

( http://youtu.be/JbqtqCunYzA)

CrashCourse Chemistry, "Effusion, Diffusion & Velocity of a

Gas" ( http://youtu.be/TLRZAFU_9Kg)


Compressibility

Expansion

Standard Temperature and Pressure


Comparing Boyles, Charles, and Gay-Lussacs Law

Study of Oxygen Lab

Using Popcorn to Determine Pressure

Generating Hydrogen Gas

Weighing by Redox

Marshmallow Peeps

Boiling Water

Heavy Newspaper

Pressure Difference

Man Your Stations Activity

gas law simulation

http://intro.chem.okstate.edu/1314F00/Laboratory/GLP.htmhttp://intro.chem.okstate.edu/1314F00/Laboratory/GLP.htm

Essential Concepts



Law, Charles’ Law, Dalton’s Law of Partial Pressures, the combined gas law, and the ideal gas law). (CHEM.B.2.2.1)

Analyze and predict the effect of making a change in one part of a system on the system as a whole. (S11.A.3.1.2)

Relate the total pressure of a mixture of gases to the partial pressures of the component gases.

3. The reference condition for gases, chosen by convention, is exactly 0°C and 1 atm pressure. (1 day)

Define standard temperature and pressure (STP).

Solutions & Their Properties (Week 33, 2 Weeks)

1. Solutions can be quantitatively described by their Molarity. (3 days)

2. Dilution is process of adding water to a more concentrated solution to

1. Solutions can be quantitatively described by their Molarity. (3 days)

Describe various ways that concentration can be expressed and calculated (CHEM.1.2.4)

Describe the effects of temperature and pressure on solubilities. (CHEM.A.1.2.3)

Textbook


Digital Media

CrashCourse Chemistry, "Water and Solutions" (http://youtu.be/AN4KifV12DA)

CrashCourse Chemistry, "Liquids" (http://youtu.be/BqQJPCdmIp8)

CrashCourse Chemistry, "Solutions" (

Concentration Calculations Quiz


Essential Concepts



lower its Molarity. (3 days)

3. The normal boiling and freezing points of a pure substance can be altered by the addition of a solute. (4 days)

Calculate molarity, solution volume, and number of moles of solute given any two of these quantities.

Compare properties of solutions containing ionic or molecular solutes (CHEM.A.1.2.1)

Calculate the concentration or mass of solute in a sample from titration data.

2. Dilution is process of adding water to a more concentrated solution to lower its Molarity. (3 days)

Calculate and perform a dilution.

Calculate the molarity of a diluted solution.

3. The normal boiling and freezing points of a pure substance can be altered by the addition of a solute. (4 days)

Describe and calculate colligative properties.

http://youtu.be/9h2f1Bjr0p4)


Molality


Dilution by Molarity

Comparing Concentrations Lab

Comparing Saturated and Unsaturated Solutions

Snow Globes

Create a Molarity Lab

Conductivity of Solutions

Acids & Bases (Week 35, 2 Weeks)

1. Acids and bases can be identified by their ability to donate/acce

1. Acids and bases can be identified by their ability to donate/accept hydrogen and/or form hydroxide ions. (3 days)

Define the

Textbook Introductory Chemistry, A Foundation; 5th Edition; Zumdahl; Chapter 15 Digital Media

Virtual pH lab

CrashCourse Chemistry, "Acid-Base Reactions in Solutions" (

Basics of pH Quiz

Unit 13 Exam Traditional Assessment:

Essential Concepts



pt hydrogen and/or form hydroxide ions. (3 days)

2. The pH scale (0-14) is used to identify an acid or base and is used to measure its relative strength. (3 days)

3. Through a neutralization reaction, a titration can be used to measure the concentration of an acid or base. (4 days)

Arrhenius idea of acid/base chemistry.

Identify ion dissociation when acids and bases are in water.

Show the formation of the hydronium ion in water.

Differentiate between strong and weak acids and bases.

2. The pH scale (0-14) is used to identify an acid or base and is used to measure its relative strength. (3 days)

The pH scale is a quantitative measure of acidity or basicity.

Locate the pH of everyday items on the pH scale.

Calculate the pH from the hydronium-ion concentration.

Calculate the hydronium-ion concentration from the pH.

Discuss ways of measuring pH and the role of acid/base indicators.

3. Through a neutralization reaction, a titration can be used to measure the concentration of an acid or base. (4 days)

http://youtu.be/ANi709MYnWg)

CrashCourse Chemistry, "pH & pOH" (http://youtu.be/LS67vS10O5Y)

CrashCourse Chemistry, "Buffers" (http://youtu.be/8Fdt5WnYn1k)


Lewis Acid and Base

Conjugate Acid Base Pairs

Bronsted Lowry

pOH

Acid Base Equilibrium


Acid Base Indicators

Titration with and Acid and Base

Determining the pH Scale

Household pH

Comparing Natural Waters/Acid Rain

Written Report

Essential Concepts



Complete a lab activity involving a titration, discussing the role of standardizing your titrant.

Calculate the pH of a solution of a strong acid and a strong base.

Define equivalence point.

Recognize that a salt is formed when an acid reacts with a base.

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